---
title: "The ionic compounds \\(\\text{LiF}\\) and \\(\\text{LiI}\\) both form crystal lattices with a \\(1:1\\) ratio of cations to anions. Which of the following correctly compares the melting points of the two compounds and provides the best justification?"
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url: "https://nerd-notes.com/ubq/119953/"
date_modified: "2026-08-21T08:24:21+00:00"
---

# The ionic compounds \(\text{LiF}\) and \(\text{LiI}\) both form crystal lattices with a \(1:1\) ratio of cations to anions. Which of the following correctly compares the melting points of the two compounds and provides the best justification?

The ionic compounds \(\text{LiF}\) and \(\text{LiI}\) both form crystal lattices with a \(1:1\) ratio of cations to anions. Which of the following correctly compares the melting points of the two compounds and provides the best justification?

- **A.** \(\text{LiI}\) has a higher melting point than \(\text{LiF}\) because \(\text{I}^-\) has more electrons than \(\text{F}^-\), resulting in stronger London dispersion forces throughout the lattice.
- **B.** \(\text{LiI}\) has a higher melting point than \(\text{LiF}\) because the larger ionic radius of \(\text{I}^-\) increases the distance between ions, which increases the lattice energy.
- **C.** \(\text{LiF}\) has a higher melting point than \(\text{LiI}\) because \(\text{F}^-\) has a smaller ionic radius than \(\text{I}^-\), resulting in shorter interionic distances and stronger electrostatic attractions.
- **D.** \(\text{LiF}\) has a higher melting point than \(\text{LiI}\) because the greater electronegativity difference produces stronger covalent bonds within the crystal lattice.

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